Question

Acids and bases:

Part I Consider the following reactions:

(a) 2 NH₃ + Ag⁺ → [Ag(NH₃)₂]⁺

(b) NH₄⁺ + CO₃^2- → NH₃ + HCO₃^-

(c) 2 HBr + Ca(OH)₂ → CaBr₂ + 2 H₂O

Match with the definitions that apply for the substances indicated. Note: In a given reaction, the same definition must apply for both the acid and base for it to hold true.

Choices:

a)Lewis-base

b)Bronsted-Lowry and Lewis Base

c) Lewis acid

d) Arrhenius, Bronsted-Lowry, and Lewis acid

e) Bronsted-Lowry and Lewis acid

f) Arrhenius, Bronsted-Lowry, and Lewis Base

Part II. Which is the stronger acid?

1) H₃PO₄ or H₂SO₄

₂₎ H₂S or (b) H₂Se

Answer 1

sol D 2NH3 + Agt -> Ing(nm),]+ Mere Ag acepts the elections son Silves is lewis acid. Anh Hill is donating its electrons to form adducts. In - Ag-in So this is lewis and a base type ran. 11) Nut + eg? → NHg at no According to Bronsted - lowry Acid-base, an and is proton donor. A base i i proton acceptor. ningt - donated not to form N43 a cor accepted proton to form nego Hence it is Bronsted-locary Acid - Base type 1) 2 HBr + calon scabra +220 Arrenhiuss which gives nt En sorrent, Bronsted done to the proton. so this equation is Arrenhius, Bronsted-lowry and lewis Base rans yee 947 ,

* 12 H₂ POqvs 1450 Audity may be define by Oxidation State. Mere H₂PO4 have phosphorous in to a.s. and 14 504 have sulphor in to o.s. so. - 1250A> POA. Acidic. H₂S vs M se. Down the group Acidity Increases as the size me. so it becomes easier to Hemove proton. so th se> AS Acidic,